How much heat is absorbed when a 10.0-g sample of water is changed from 23.0⁰C to 32.0⁰C?

376.56J

Explanation:

The amount or quantity of heat absorbed can be calculated using the formula:

Q = m × c × ∆T

Where; Q = amount of heat absorbed (J)

m = mass of water (g)

c = specific heat capacity of water (J/g°C)

∆T = change in temperature (°C)

According to the provided information in this question; m = 10.0g, c = 4.184J/g°C, final temperature = 32°C, initial temperature = 23°C

Q = m × c × ∆T

Q = 10 × 4.184 × (32 - 23)

Q = 41.84 × 9

Q = 376.56J

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

answer: any goods being imported from another country may be subject to issued by the federal government are tariffs

explanation:  

tariffs are a tax on anything that are imported from abroad. government use them to protect and boost their local industries and the thought is that they encourage consumers to buy local instead of importing and they will hope will protect jobs and economy in the country that implements them